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Test Review # 6

Chemistry R: Form TR6-9A Name _____REVIEW Date _____ Period _____Test Review # 6 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing thesymbol, the atomic mass, and the chemical properties. He arranged the cards in order of increasing atomic mass and noticeda pattern: MENDELEEV'S PERIODIC LAW When the elements are arranged in increasing order of atomic mass, the chemicalproperties repeat themselves periodically. Moseley noticed that when all the elements were arranged in order of mass a few werenot in the right family with respect to properties.

Chemistry R: Form TR6.9A Test Review # 6 REVIEW Page 2 7. Most of the elements in the Periodic Table are classified as (1) metalloids, (2) nonmetals, (3) noble gases, (4) metals

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1 Chemistry R: Form TR6-9A Name _____REVIEW Date _____ Period _____Test Review # 6 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing thesymbol, the atomic mass, and the chemical properties. He arranged the cards in order of increasing atomic mass and noticeda pattern: MENDELEEV'S PERIODIC LAW When the elements are arranged in increasing order of atomic mass, the chemicalproperties repeat themselves periodically. Moseley noticed that when all the elements were arranged in order of mass a few werenot in the right family with respect to properties.

2 He used a procedure called X-ray diffraction to determine the atomic numberof the elements. When the elements were arranged in increasing order of atomic number, the discrepancies in Mendeleev's tabledisappeared. THE PERIODIC LAW When the elements are arranged in increasing order of atomic number, the chemicalproperties repeat themselves periodically. The modern Periodic Table is arranged in order of increasing atomic of the Periodic Table. The modern Periodic Table is arranged in order of increasing atomic number in verticalcolumns and horizontal rows. The vertical columns are elements with about the same number of outer electrons (valenceelectrons).

3 They are called groups or families. Elements in the same family have similar properties. Horizontal rows areelements with the same number of shells or energy levels. They are called periods. The major divisions of the Periodic Tableare: Alkali metals - Group 1; Alkaline earth metals - Group 2; Halogens - Group 17; Noble gases (Inert gases) - Group 18;Transition metals - Groups 3-12; Lanthanides - Row 6, elements 57 - 71;and Actinides - Row 7, elements 89 - in the Periodic Table. Going across the table from left to right within a row or period the number of protonsincreases, so the pull on the electrons increases.

4 As a result the covalent atomic radius decreases and metallic propertiesdecrease (except in the transition elements). In addition the number of valence electrons increases and the number of shellsremains the same. Going down the table within a group or family the number of protons also increases, but the number ofshells increases too. As a result, the atomic radius increases, the pull on the electrons decreases, and metallic propertiesincrease. In a family the number of valence electrons remains the same. This results in the following organization of thePeriodic Table:Answer the questions below by circling the number of the correct response1.

5 In the Periodic Table, the elements are arranged in order ofincreasing (1) atomic size, (2) atomic number, (3) atomic mass,(4) ionization energy2. The chemical properties of the elements are periodic functions oftheir atomic (1) spin, (2) isotopes, (3) mass, (4) Which pair contains elements which have the most similar chemicalproperties? (1) Mg and Ca (2) N and S (3) H and Li (4) Na and Cl4. The element with an atomic number of 34 is most similar in itschemical behavior to the element with an atomic number of (1) 19(2) 31 (3) 36 (4) 165. Silicon is most similar in chemical activity to (1) carbon, (2) lead,(3) sulfur, (4) nitrogen6.

6 The element 2 8 6 belongs in Period (1) 6, (2) 2, (3) 3, (4) 411811M12 13141516172N2O23E2-142-252-362-472-582-6 9N2-7O10B2-8L311T2-8-1122-8-2132-8-3142- 8-4152-8-5162-8-617N2-8-7M18E2-8-8419A2- 8-8-1202-8-8-2 ETGA5 LALSE6 SSS7 Chemistry R: Form Review # 6 REVIEWPage 27. Most of the elements in the Periodic Table are classified as(1) metalloids, (2) nonmetals, (3) noble gases, (4) metals8. Phosphorus is best classified as a (1) nonmetal , (2) metalloid ,(3) metal , (4) transition element9. The Group 1 metals all have the same (1) electronegativity,(2) atomic radius, (3) oxidation state, (4) ionization energy10.

7 Which Group in the Periodic Table contains the most active metals? (1) 1 (2) 2 (3) 13 (4) 1411. In which Group of the Periodic Table would this element, 2 5, mostlikely be found? (1) 1 (2) 2 (3) 13 (4) 1512. As the elements in Period 3 are considered in order of increasingatomic number, the number of principal energy levels in eachsuccessive element (1) decreases (2) increases (3) remains thesame13. Which Group contains elements which are metalloids? (1) 1 (2) 11(3) 14 (4) 414. The elements with the least chemical reactivity are in Group (1) 1,(2) 18, (3) 3 (4) 1615. Which element is a metalloid ?

8 (1) arsenic (2) neon (3) potassium(4) bromine16. Which Group of elements exhibits all three phases of matter at roomtemperature? (1) 2 (2) 14 (3) 15 (4) 1717. What are two properties of most nonmetals?(1)high ionization energy and poor electrical conductivity(2) high ionization energy and good electrical conductivity(3) low ionization energy and poor electrical conductivity(4)low ionization energy and good electrical conductivity18. Which element is classified as a noble gas at STP? (1) hydrogen(2) neon (3) oxygen (4) nitrogen19. In which shell are the valence electrons of the elements in Period 2found?

9 (1) 1 (2) 2 (3) 3 (4) 420. Of the following, which element has the smallest atomic radius?(1) Mg (2) Ca (3) Sr (4) Ba21. As one proceeds from lithium to fluorine in the Periodic Table, thetendency for the elements to lose electrons (1) decreases,(2) increases, (3) remains the same22. As the elements in Period 3 are considered from left to right, theability of each successive element to gain electrons (1) decreases,(2) increases, (3) remains the same23. Of the following, which is the element with the most metalliccharacter in Group 16 is (1) O, (2) S, (3) Se, (4) Te24.

10 As the elements in Group 14 are considered in order of increasingatomic number, the metallic properties of successive elements(1) decreases, (2) increases, (3) remains the same25. In Period 3 of the Periodic Table, the element with the smallestatomic radius is in Group (1) 1 (2) 2 (3) 15 (4) 1726. Of the following, which Group 2 element has the greatest tendency tolose electrons? (1) calcium (2) barium (3) strontium (4) magnesium27. Which Group in the Periodic Table contains atoms that have anoxidation state of 2? (1) 1 (2) 2 (3) 16 (4) 1728. The elements in Group 2 have similar chemical properties primarilybecause they have the same (1) ionization energies, (2) reductionpotentials, (3) number of principal energy levels, (4) number ofelectrons in the outermost shell29.


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